1. Solubility
Review

2. 1. Solubility is a measure of the maximum amount of solid that
1. Solubility is a measure of the maximum amount of solid that will dissolve in a volume of water.
Units: g/L mol/L g/100mL
Or even: mL/L for CO2(g) in water
Ksp
Solubility Product
Saturated solutions
No Units
Only Changes with Temperature
No ICE!
Step #1 Write a dissociation equation for the low solubility salt

3. 2. The solubility (s) of BaCO3 is 5. 1 x 10-5 M @ 250 C. Calculate the
2. The solubility (s) of BaCO3 is 5.1 x C. Calculate the solubility product or Ksp.
Dissociation net ionic BaCO3(s) ⇌ Ba CO32-
s s s
Ksp = [Ba2+][CO32-]
Ksp = s2
Ksp = (5.1 x 10-5)2
Ksp = x 10-9
Adding BaCO3 does not increase [Ba2+] or [CO32-] but it does increase the rate of dissolving and crystallization.
Formation Net Ionic: Ba CO32-  BaCO3(s)
Ba2+
CO32-
BaCO3(s)

4. 2. The solubility (s) of BaCO3 is 5. 1 x 10-5 M @ 250 C. Calculate the
2. The solubility (s) of BaCO3 is 5.1 x C. Calculate the solubility product or Ksp.
BaCO3(s) ⇌ Ba CO32-
s s s
Ksp = [Ba2+][CO32-]
Ksp = s2
Ksp = (5.1 x 10-5)2
Ksp = x 10-9
Adding BaCO3 does not increase [Ba2+] or [CO32-] but it does increase the rate of dissolving and crystallization.
Formation Net Ionic: Ba CO32-  BaCO3(s)
Ba2+
CO32-
BaCO3(s)

5. 3. PbCl2(s) ⇌ Pb Cl-
Ksp = s3

6. 4. 200. 0 mL 0. 10 M Pb(NO3)2 is mixed with 300. 0 mL of 0. 20 M
mL 0.10 M Pb(NO3)2 is mixed with mL of 0.20 M NaCl, will a precipitate occur?
PbCl2(s) ⇌ Pb Cl-
M M
0.040 M M
TIP = [Pb2+][Cl-]2
TIP = [0.040][0.12] 2
= 5.8 x 10-4
Ksp = 1.2 x TIP > Ksp ppt forms

7. 5. Changing the Solubility of a Salt E + Ca(OH)2(s) ⇄ Ca2+ + 2OH-
E + Ca(OH)2(s) ⇄ Ca OH-
Substance Added Effect on Molar Solubility Effect on Ksp
Ca(NO3)2 Decrease none
Na2SO4 Increase none
NaOH Decrease none
HCl Increase none
NaCl none none
Ca(OH)2 none none
Increase Temperature Increase Increase
Decrease Temperature Decrease Decrease

8. 6. Mg(OH)2 will have the greatest solubility in:
Mg(OH)2(s) ⇌ Mg OH-
A. NaOH OH- lowers solubility
B. Mg(NO3)2 Mg2+ lowers solubility
C. H2O No effect solubility
D. AgNO3 Ag+ increases solubility by reacting with OH-

9. 7. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution.
AgCl(s) ⇄ Ag Cl-
0.20 M
Ksp = [Ag+][Cl-]
1.8 x = [0.20][Cl-]
[Cl-] = 9.0 x M
BaCl2(s) ⇄ Ba Cl-
4.5 x M x M
0.50 L x x mole x g = x g
1 L mole

10. 8. Ionic Solutions: NaCl HCl NH4NO3
Molecular Solutions: C12H22O11
9. What is the answer?
A. NaCl
B. CaCl2
C. AgCl
D. AgBr

11. 10. Ionic Solutions: NaCl HCl NH4NO3
Molecular Solutions: C12H22O11
11. What is the answer?
A. NaCl High
B. CaCl2 High
C. AgCl Low x
D. AgBr Low x